For the reaction $A + B \to C$,it is found that doubling the concentration of $A$ increases the rate by $4$ times,and doubling the concentration of $B$ doubles the reaction rate. What is the overall order of the reaction?

If a reaction occurs in the following two steps:
$i) \ 2 ClO^{-} \rightarrow ClO_2^{-} + Cl^{-}$
$ii) \ ClO_2^{-} + ClO^{-} \rightarrow ClO_3^{-} + Cl^{-}$
Find the reaction intermediate.

The rate constant of esterification is given by $k = k^{\prime} [H_2O]$. If the rate constant $k = 2.0 \times 10^{-3} \ min^{-1}$,calculate $k^{\prime}$. (Assume $[H_2O] = 55.5 \ mol \ L^{-1}$)

For a reaction $r = k[A][B]^2$,if the concentration of $A$ is doubled,the rate of reaction:

For the reaction $A + B \rightleftharpoons AB$,if the concentrations of both $A$ and $B$ are doubled,the rate of the reaction will become .......

The number of incorrect statement/s from the following is:
$A$. The successive half-lives of zero-order reactions decrease with time.
$B$. $A$ substance appearing as a reactant in the chemical equation may not affect the rate of reaction.
$C$. Order and molecularity of a chemical reaction can be a fractional number.
$D$. The rate constant units of zero and second-order reactions are $mol \ L^{-1} s^{-1}$ and $mol^{-1} L s^{-1}$ respectively.